chapter 3 ~ chemical reactions
DESCRIPTION
Chapter 3 ~ Chemical Reactions. Balancing Combustion Reactions. Write a balanced equation for the combustion of butane. Chemical Equilibrium. Solution Terms. Solvent Solute Homogeneous mixture Aqueous Electrolyte (strong / weak) Nonelectrolyte. - PowerPoint PPT PresentationTRANSCRIPT
Chapter 3 ~ Chemical Reactions
Balancing Combustion ReactionsWrite a balanced equation for the
combustion of butane.
Chemical Equilibrium
Solution Terms• Solvent• Solute• Homogeneous mixture• Aqueous• Electrolyte (strong / weak)• Nonelectrolyte
Solubility of Ionic Compounds in Water
Exercise 3.4 ~Predict the solubility of the following
compounds:
LiNO3
CaCl2
CuONaC2H3O2
List as many types of chemical reactions as you can.
Give an example of each type of reaction
Precipitation Reactions aka: Double Replacement Rxns
Exercise 3.5 ~ Will precipitation reactions occur between:
Sodium carbonate and copper (II) chloride
Potassium carbonate and sodium nitrate
Nickel(II) chloride and potassium hydroxide
Writing Net Ionic EquationsExercise 3.6Write balanced net ionic equations for:Aluminum chloride and sodium
phosphate
Iron(III) chloride and potassium hydroxide
Lead(II) nitrate and potassium chloride
Acid / Base ReactionsCharacteristics of Characteristics
of Acids Bases
HCl + Zn
Using the Activity Series
Al + CuCl2
Cu + NaCl
Zn + HCl
Cu + HCl
Ca + H2O
Naming Acids
Binary Acids
Oxyacids
Acids and BasesDefinitions:Arrhenius Acid: an acid is a substance that
ionizes in water to produce H+ or H3O+ ionsHCl + H2O
Arrhenius Base: a base produces OH- ions in water
NaOH
Bronsted-Lowry Acids and BasesAcid: a substance that donates a proton to
any other substanceBase: a substance that accepts a proton
from another substanceHNO3 + H2ONH4
+ + H2OFe(H2O)6
3+ + H2O
NH3 + H2O
Amphiprotic Substances
Act as a Bronsted acid OR a Bronsted baseHCO3 + H2O H3O+ + CO3
2-
OR HCO3 + H2O H2CO3 + OH-
Conjugate Acid-Base Pairs
HCO3 + H2O H3O+ + CO32-
Conjugate acid-base pairs differ by the presence of a _____________________________
Ionization of Acids and Bases
Strong Acids
Weak Acids
Diprotic and polyprotic acids
Ionization of bases
Common Acids and Bases
Metal and Nonmetal Oxides
• CO2• SO2• SO3• NO2• CaO• MgO
Reactions of Strong Acids and Strong Bases
HCl + NaOH
HNO3 + NaOH
H2SO4 + Ca(OH)2
Mg(OH)2 + HCl
Reactions of Weak Acids
• Acetic Acid and sodium hydroxide
Gas Forming Reactions
Acids + CarbonatesCalcium carbonate + HCl
Calcium carbonate + HC2H3O2
Acids + bicarbonatesNaCO3 + HC4H5O6
Gas Forming Reactions
• Acids + sulfidesNa2S + HCL
Gas Forming Reactions
• Acids + sulfitesNa2SO3 + HCl
• Ammonium salts + basesNH4Cl + NaOH
Exercise 3.11
Write the equation for the reaction of barium carbonate and nitric acid
Write a balanced equation for the reaction of ammonium sulfate and sodium hydroxide
Driving Forces for Reactions
• Precipitation Reactions
• Gas forming reactions
• Acid-base reactions
• Oxidation-reduction reactions
TEST TUBE WITH NAIL -OBSERVATIONS:
EXPLANATIONS?????
CuSO4 and NaCl combine:
Activity Series: Fe, Cu
Iron ions react with oxygen and water:
New Concepts:
Complex ion ~
Redox Reactions ~
Base Anhydride ~
Oxidation Numbers
• As opposed to valence number:
Rules for Assigning Oxidation Numbers1. Pure elements have oxidation numbers of 02. Single element ions have oxidation numbers
equal to their charges3. F always an oxidation number = -14. Cl, Br, I always = -1 except in compounds with
O or F5. H has an oxidation number of +1 unless it is a
hydride ion (-1)6. O has an oxidation number of -2 unless it is a
peroxide (-1) or superoxide7. Oxidation numbers of elements in polyatomic
ions always = the charge of the ion8. Oxidation numbers in compounds always add
to 0.
Determining Oxidation Numbers
• Fe2O3
• CO32-
• H2SO4
• NO21+
Oxidation-Reduction Reactions
Fe2O3(s) + 3CO(g) 2Fe(s) + 3CO2(g)
Redox Reactions
• Element oxidized
• Element reduced
• Oxidizing agent
• Reducing agent
Breathalyzer Reaction
3CH3CH2OH + 2Cr2O72- + 16 H3O+
3CH3CO2H + 4 Cr3+ +27H2O
9 Oxidation States of N
• NO31- NO2
• NH4 1+ N2H4
• NH2OH N2
• N2O NO• N2O3
H2O2 + Blood
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